Abstract. In this present paper, cuprous-oxide (Cu2O) nanoparticles were successfully fabricated using
ascorbic acid as a reducing agent. The purity and characteristics of Cu2O nanoparticles were determined
with XRD and FT-IR techniques. The morphology and particle size of the material were characterized
using SEM and TEM, respectively. The results show that the concentration of sodium hydroxide affects
the morphology and particle size of the material. Furthermore, the Cu2O nanoparticles with a particle
size of 70–80 nm exhibit good photocatalytic activity on photodegradation of Rhodamine B under visible
light, and the photocatalytic degradation ratio of Rhodamine B is 70%.
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Hue University Journal of Science: Natural Science
Vol. 128, No. 1D, 31–37, 2019
pISSN 1859-1388
eISSN 2615-9678
DOI: 10.26459/hueuni-jns.v128i1D.5372 31
PREPARATION OF CUPROUS-OXIDE NANOPARTICLES USING
ASCORBIC ACID AS REDUCING AGENT AND ITS
PHOTOCATALYTIC ACTIVITY
Dang Xuan Du*, Pham Thi Giang Anh
Faculty of Pedagogy in Natural Sciences, Sai Gon University, 273 An Duong Vuong St., Ward 3, District 5,
Ho Chi Minh City, 700000, Vietnam
* Correspondence to Dang Xuan Du
(Received: 19 August 2019; Accepted: 12 October 2019)
Abstract. In this present paper, cuprous-oxide (Cu2O) nanoparticles were successfully fabricated using
ascorbic acid as a reducing agent. The purity and characteristics of Cu2O nanoparticles were determined
with XRD and FT-IR techniques. The morphology and particle size of the material were characterized
using SEM and TEM, respectively. The results show that the concentration of sodium hydroxide affects
the morphology and particle size of the material. Furthermore, the Cu2O nanoparticles with a particle
size of 70–80 nm exhibit good photocatalytic activity on photodegradation of Rhodamine B under visible
light, and the photocatalytic degradation ratio of Rhodamine B is 70%.
Keywords: cuprous-oxide nanoparticles, ascorbic acid, photocatalytic degradation, photocatalytic
activity, Rhodamine B
1 Introduction
Cu2O with a small band gap of about 2 eV [1] is a p-
type semiconductor. It is considered as a promising
material in electronics, solar energy conversion, and
catalysis [2, 3]. According to Hu et al., the conductive
degree of the pastes-copper powder depends on the
morphology and size of the Cu2O precursor [4].
Varying efforts have also been devoted to the
preparation of Cu2O with various morphologies such
as cube [5, 6], sphere [7, 8], tubular-like [5], and
octahedron [9, 10]. Nevertheless, the majority of
approaches utilize inconvenient techniques such as
irradiation of microwave [6, 8] or organic additive as
modifier [5, 7]. In this study, Cu2O nanoparticle was
prepared by reducing Cu (II) in alkaline media using
ascorbic acid as a reducing agent without a template.
The influence of the NaOH concentration on the
shape of Cu2O nanoparticles was investigated.
Furthermore, its photocatalytic activity in
photodegradation of Rhodamine B under visible light
was also studied.
2 Experimental
2.1 Materials
Copper sulfate (CuSO4.5H2O), ascorbic acid
(C6H8O6), sodium hydroxide (NaOH) purchased
from Beijing Chemical Reagent Company, and
ethanol as a solvent were of analytical grade and
were used without further purification.
2.2 Preparation of Cu2O nanoparticles
In different sequences of the experiment, the
volumes of CuSO4, NaOH, and C6H8O6 solutions
were kept constant at 20, 40, and 50 mL,
respectively. The concentration of CuSO4 and
Dang Xuan Du and Pham Thi Giang Anh
32
ascorbic acid is 0.5 and 0.1 M, respectively.
Whereas, the concentration of NaOH is 0.5, 1.0, and
1.5 M.
Firstly, the precursor was prepared by
dropping 40 mL of NaOH solution into 20 mL of
the CuSO4 solution under stirring in a 200 mL flask
at room temperature. Secondly, 50 mL of the
ascorbic acid solution was added into the mixture
by dropping on the surface of the precursor
solution under vigorous stirring to form a brick-
red mixture with stable colour. Finally, the
products were collected by centrifugation, washed
five times with distilled water and three times with
ethanol, and then dried at 60 °C for 24 h [11].
The XRD study of the powder was carried
out using an X-ray diffractometer (D8 Advance,
Bruker, Germany) with Cu Kα radiation (λ = 1.541
Å). The morphology and particle size of the Cu2O
nanoparticles were investigated using SEM
(Hitachi S4800, Japan) and TEM (JEM 1400, JEOL,
Japan). The FTIR spectra of the material were taken
on an FT-IR 8400S spectrometer (Shimadzu, Japan)
using KBr pellets.
2.3 Photocatalytic degradation of
Rhodamine B
0.1 g of Cu2O powder with a particle size of 76 nm
was added to a 200 mL flask containing 100 mL of
a RhB (Beijing, China) solution with a
concentration of 2 mg/L. Cu2O is dispersed in the
solution with vigorous stirring. The whole system
is placed under sunlight or the light of a mercury
lamp (E27-125 W) for 4 hours. The sample was
taken every 30 minutes to determine the
transmittance of the solution. The sample is
centrifuged at a rate of 1000 rpm for 15 minutes to
remove the catalyst before UV-VIS measurement.
The degree of degradation of RhB was calculated
according to the following formula
0
0
(%) 100
C C
C
−
=
where C0 and C are the initial concentration of
RhB and the concentration of RhB at the time of
taking the sample, respectively [10].
3 Results and discussion
3.1 Formation of Cu2O nanoparticles
As shown in Fig. 1, there is a change in colour dur-
ing the reaction. It is obvious that the initial solu-
tion (CuSO4) is blue and transparent (Fig. 1a).
When NaOH was added, the colour of the reaction
mixture became brick-red, the characteristic colour
of Cu(OH)2 (Fig. 1b). The brick-red characteristic
colour of Cu2O appeared after ascorbic acid was
dumped into the reaction mixture (Fig. 1c). In this
process, Cu2+ ions are reduced by ascorbic acid to
form Cu2O nanoparticles. The reactions are as fol-
lows [11]:
Cu2+ + 2OH– → Cu(OH)2 (1)
2Cu(OH)2 + C6H8O6 → Cu2O + C6H6O6 + 3H2O (2)
The total reaction is
2Cu2+ + C6H8O6 + 4OH – → Cu2O + C6H6O6 + 3H2O (3)
Fig. 1. CuSO4 solution (a), CuSO4 solution with NaOH (b), and reaction mixture with ascorbic acid (c)
Hue University Journal of Science: Natural Science
Vol. 128, No. 1D, 31–37, 2019
pISSN 1859-1388
eISSN 2615-9678
DOI: 10.26459/hueuni-jns.v128i1D.5372 33
3.2 Characterization of Cu2O
nanoparticles
As shown in Fig. 2, the colour of the Cu2O nano-
particles in the reaction mixture and the powder
state (inset in the figure) became darker with the
NaOH concentration. This result may be due to the
enhancement of the particle size (Table 1). The
XRD patterns of the Cu2O products are shown in
Fig. 3. On the diffraction patterns, the Cu2O prod-
ucts prepared with different concentrations of
NaOH have characteristic peaks at 29.61°, 36.48°,
42.38°, 61.46°, 73.56°, and 77.52° corresponding to
(110), (111), (200), (210), (311), and (222) plane of
Cu2O. These patterns indicate that the products are
pure Cu2O because no peaks of Cu and CuO are
observed [9, 12].
Fig. 2. Colour of Cu2O in reaction mixture and in powder state with different NaOH concentrations: 0.5 M (a),
1.0 M (b), and 1.5 M (c)
Fig. 3. XRD patterns of Cu2O nanoparticles prepared with different NaOH concentrations: 0.5 M (a), 1.0 M (b),
and 1.5 M (c)
Dang Xuan Du and Pham Thi Giang Anh
34
As shown in Fig. 4, the FI-IR spectra of all
Cu2O products prepared with different
concentrations of NaOH show a peak at 623 cm–1
corresponding to the Cu–O bond of the Cu2O
crystal [13, 14]. The FI-IR spectra also reveal that
there is a slight shift to lower wavenumber as
NaOH concentration increases. This may be due to
the decrease in particle size (Table 1).
Fig. 4. FT-IR spectra of Cu2O nanoparticles prepared with different NaOH concentrations: 0.5 M (a), 1.0 M (b),
and 1.5 M (c)
Table 1. Size of Cu2O particles prepared with different concentrations of NaOH
Note NaOH concentration (mol/L) Size of Cu2O (nm)
a 0.5 71
b 1.0 76
c 1.5 80
Hue University Journal of Science: Natural Science
Vol. 128, No. 1D, 31–37, 2019
pISSN 1859-1388
eISSN 2615-9678
DOI: 10.26459/hueuni-jns.v128i1D.5372 35
Fig. 5. TEM images and size distribution histogram of Cu2O nanoparticles prepared with different concentrations of
NaOH: 0.5 M (A, a); 1.0 M (B, b), and 1.5 M (C, c)
As shown in Fig. 5, the TEM image and
distribution histogram of Cu2O nanoparticles
prepared with NaOH concentration of 0.5 M (A, a)
reveal that the Cu2O particles have a spherical
shape in the cluster state with a particle diameter
of about 71 nm, and the particle size ranges from
30 to 89 nm with a nearly normal distribution.
When the NaOH concentration is 1.0 M, the
Dang Xuan Du and Pham Thi Giang Anh
36
particle diameter is 76 nm, and the particle size
ranges from 17 to 89 nm with a nearly normal
distribution. A different distribution is observed
when the NaOH concentration is 1.5 M, and the
particle size ranges from 70 to 130 nm with the
mean of particle size of about 80 nm. When the
concentration of NaOH increases, the Cu2O
nanoparticles tend to cluster, forming large
particles with an octahedron shape (Fig. 5C). The
mechanism for the formation of nanoparticle
shapes via changing the concentration of NaOH
was mentioned by Wang et al. [11]. According to
this study, the shapes of the nanoparticles depend
on the adsorbed quantity of the OH– ions on the
surface of the Cu2O particles. When the
concentration of NaOH is low, the adsorbed
quantity of OH– ions on the surface of Cu2O
particles is relatively small. Therefore, when the
repulsion between single nuclei, primary particles,
and molecule clusters is weak, aggregation is the
overwhelming growth mode, and the crystal nuclei
grow into spherical particles as a result of
aggregation. When the concentration of NaOH
increases, the adsorbed quantity of OH– ions on the
surface of Cu2O particles is greater. This leads to
the repulsion among primary particles, restraining
the aggregation growth mode. Moreover, the high
density of OH– on the (111) facet restrains the
growth of this (111) facet [11]. As a result, the
morphology of Cu2O is mostly octahedral.
3.3 Photocatalytic performance
Fig. 6 depicts the degradation of RhB on Cu2O
nanoparticles with a size of 76 nm under sunlight
and mercury light. It can be seen that the degree of
degradation of RhB under sunlight is smaller than
that under mercury light at 60 and 70%,
respectively. It could be concluded that the
degradation of RhB has a lower efficiency under
sunlight compared with mercury light. However,
for a large-scale application, sunlight should be
chosen because of the low cost and convenient
equipment
4 Conclusions
A facile chemical approach with ascorbic acid as a
reducing agent without a template was developed
to prepare Cu2O nanoparticles. The experiments
show that pure Cu2O nanocrystals were efficiently
synthesized in the alkali media, and the
concentration of NaOH has an impact on the
particle size of the material. Cu2O nanoparticles
with a particle size of 76 nm have a good
photocatalytic activity on photodegradation of
RhB with degradation ratio of RhB reaching to 70%
under visible light.
Funding statement
This study was supported by the Research Grant of
Sai Gon University with Key Project CS2017-05.
Fig. 6. Degradation of RhB under visible light: sunlight and mercury light
Hue University Journal of Science: Natural Science
Vol. 128, No. 1D, 31–37, 2019
pISSN 1859-1388
eISSN 2615-9678
DOI: 10.26459/hueuni-jns.v128i1D.5372 37
Conflict of interests
The authors declare that there is no conflict of
interest regarding the publication of this article.
Acknowledgement
The authors would like to thank Professor N. Q.
Hien (VINAGAMMA Center, VINATOM
Vietnam) for reading this manuscript.
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